Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of benzoic acid (p?a=4.20) and 40.0 mmol of benzoate. Calculate the pH of this buffer. What volume of 3.50 M NaOH would be required to increase the pH to 4.93?

A chemistry graduate student is given 450. mL of a 0.50M methylamine (CH, NH,) solution. Methylamine is a weak base with K,=4.4 × 10 *. What mass of CH,NH,Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH = 10.96? You may assume that the volume of the solution doesn't change when the CH,NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. olo x10 Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility .........................................

Ka of glycolic acid is 1.47 x 10^-4

An analytical chemist is titrating 234.0 mL of a 0.4400M solution of butanoic acid (HC,H,CO,) with a 0.3900M solution of NaOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 63.61 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places.

The buffer was made by combining 0.220 M lactic acid (HC3H5O3) and 0.200 M sodium lactate ( NaC3H5O3). The Ka of HC3H5O3 is 1.4 x 10^-4. 1. write the equation describing the conjugate acid base relationship 2. Calculate the pH of the buffer 3. Calculate the pH of the buffer after the addition of 100.0 mL of 0.100 M potassium hydroxide to 0.9000 L of the buffer solution

Please calculate the pH of a buffer solution made up of citric acid and potassium citrate. The solution was made by dissolving 0.770 mol of sodium citrate, and 0.770 mol of citric acid in 1.5 liters of water. (Please assume the total volume of the solution is also 1.5 L) (The Ka for this system = 7.41 x 10-4) (Please answer with 3 sig. figs.)